Using the half-reaction method and showing all of your steps, write the balanced equation for the oxidation-reduction reaction between manganese(II) ions and periodate in acidic solution. Be sure to show each step when balancing each half-reaction, as well as how the electrons balance between the two half-reactions.

I need number 3 answers and conclusions

1.         With reference to the following list, which of the statements is true? The following is a list of some of the metals in the galvanic series in their relative order: -               Anode end -               Tin -               Zinc -               Copper -               Aluminium -               Nickel -               Cadmium -               Titanium -               Mild Steel -               Platinum -               Cast Iron -               Cathode End ¨   copper is more corrodible than mild steel if they are in contact ¨   aluminium and nickel together have  greater  corrosion potential than aluminium and tin ¨   platinum is the most corrodible metal ¨   zinc is the least corrodible metal

[Review Topics] [References] Use the References to access important values if needed for this question. Fe2+ + Ni→Ni²* + Fe In the above redox reaction, use oxidation numbers to identify the element oxidized, the element reduced, the oxidizing agent and the reducing agent. name of the element oxidized: name of the element reduced: formula of the oxidizing agent: formula of the reducing agent: Submit Answer Retry Entire Group 6 more group attempts remaining Previous Next Email Instructor Save and

Nhen zinc metal is added to a beaker of hydrochloric acla, a gas is produced. Write the balanced net ionic equation for this reaction. Write the oxidation and reduction half reactions. What quantity of useful work can be obtained when Zn is added directly to the beaker of HCI? How can you harness this reaction to do useful work? Draw a diagram that shows this.

Write the half-reaction that occurs at the anode during the electrolysis of NaCl. Include physical states and use single arrow in your equation. Incorrect. Recall that reduction takes place at the cathode, so the substance must be gaining electrons. Write the half-reaction that occurs at the cathode during the electrolysis of NaCl. Include physical states and use single arrow in your equation. Incorrect. Is your reaction balanced? There should be no electrons in a balanced final equation. Write the overall cell reaction for the electrolysis of NaCl. Include physical states and use single arrow in your equation.